Question

The volume of a gas is 450 mL when its pressure is 1.00 atm. If the temperature of the gas does not change, what is the pressure when its volume is changed to 2.00 L?
Use .
0.225 atm
0.444 atm
2.25 atm
4.44 atm

Answer 1

Answer: The pressure of the gas is 0.225 atm.

Explanation: To calculate the pressure of the gas, we use Boyle's Law.

Boyle's Law states that pressure is inversely proportional to the volume of the gas at constant temperature.

Mathematically,

$P\propto \frac{1}{V}$

Or,

$P_1V_1=P_2V_2$

where,

$P_1\text{ and }V_1$ are the initial pressure nd volume.

$P_2\text{ and }V_2$ are the final pressure andvolume

Initial conditions:

$P_1=1atm\\V_1=450mL$

Final conditions:

$P_2=?atm\\V_2=2L=2000mL$

Conversion factor: 1L = 1000mL

Putting values in above equation, we get:

$1atm\times 450mL=P_2\times 2000mL\\P_2=0.225atm$

Answer 2

At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 =P2V2

P2 = P1 x V1 / V2

P2 = 1 x .450 / 2

P2 =.225 atm

Hope this answers the question. Have a nice day.